Sal volatile | Define Sal volatile at Dictionary.com sal volatile [sal voh-lat-l-ee] /ˈsæl voʊˈlæt lˌi/ Spell an aromatic alcoholic solution of ammonium carbonate, the chief ingredient in smelling salts. Origin of sal volatile 1645-55; < New Latin: volatile salt Dictionary.com Unabridged Examples from the Web for sal volatile Expand Historical Examples The Guardian Angel Oliver Wendell Holmes, Sr. An uneasy conscience?ah!for an uneasy conscience there is nothing better than sal volatile! The Lamp of Fate Margaret Pedler A few drops (15 to 30) of ether, with a little tincture of capsicum or spirit of sal volatile, seldom fail to give relief. British Dictionary definitions for sal volatile Expand another name for ammonium carbonate 2. Also called spirits of ammonia, (archaic) hartshorn. a solution of ammonium carbonate in alcohol and aqueous ammonia, often containing aromatic oils, used as smelling salts Word Origin C17: from New Latin: volatile salt Collins English Dictionary - Complete & Unabridged 2012 Digital Edition © William Collins Sons & Co. Ltd.

1979, 1986 © HarperCollins Publishers 1998, 2000, 2003, 2005, 2006, 2007, 2009, 2012 Word Origin and History for sal volatile Expand n. 1650s, Modern Latin, literally "volatile salt" (see salt (n.) + volatile ); ammonium carbonate, especially as used in reviving persons who have fainted. Online Etymology Dictionary, © 2010 Douglas Harper People invent new words all the time, but which ones actually make it? Word of the Day Spirit of hartshorn | Article about Spirit of hartshorn by The Free Dictionary Spirit of hartshorn | Article about Spirit of hartshorn by The Free Dictionary Also found in: Dictionary , Thesaurus , Medical , Wikipedia . ammonia, chemical compound, NH3, colorless gas that is about one half as dense as air at ordinary temperatures and pressures. It has a characteristic pungent, penetrating odor.

Ammonia forms a minute proportion of the atmosphere; it is found in volcanic gases and as a product of decomposition of animal and vegetable matter. Because ammonia was formerly obtained by destructive distillation of horns and hooves of animals, its water solution was called spirits of hartshorn. Ammonia has also been called alkaline air and volatile alkali. Properties Anhydrous (water-free) ammonia gas is easily liquefied under pressure (at 20&degC; liquid ammonia has a vapor pressure of about 120 lb per sq in.) It is extremely soluble in water; one volume of water dissolves about 1,200 volumes of the gas at 0&degC; (90 grams of ammonia in 100 cc of water), but only about 700 volumes at room temperature and still less at higher temperatures. The solution is alkaline because much of the dissolved ammonia reacts with water, H2O, to form ammonium hydroxide, NH4OH, a weak base. Liquid ammonia is used in the chemical laboratory as a solvent.

It is a better solvent for ionic and polar compounds than ethanol, but not as good as water; it is a better solvent for nonpolar covalent compounds than water, but not as good as ethanol. It dissolves alkali metals and barium, calcium, and strontium by forming an unstable blue solution containing the metal ion and free electrons that slowly decomposes, releasing hydrogen and forming the metal amide. Compared to water, liquid ammonia is less likely to release protons (H+ ions), is more likely to take up protons (to form NH4+ ions), and is a stronger reducing agent. Because strong acids react with it, it does not allow strongly acidic solutions, but it dissolves many alkalies to form strongly basic solutions. Ammonia takes part in many chemical reactions. Ammonia reacts with strong acids to form stable ammonium salts: with hydrogen chloride it forms ammonium chloride ammonium chloride , chemical compound, NH4Cl, a white or colorless, odorless, water-soluble, cubic crystalline salt with a biting taste, commonly known as sal ammoniac. ..... Click the link for more information.

; with nitric acid, ammonium nitrate ammonium nitrate, chemical compound, NH4NO3, that exists as colorless, rhombohedral crystals at room temperature but changes to monoclinic crystals when heated above 32&degC;. It is extremely soluble in water and soluble in alcohol and liquid ammonia. ..... Click the link for more information. ; and with sulfuric acid, ammonium sulfate ammonium sulfate, chemical compound, (NH4)2SO4, a colorless-to-gray, rhombohedral crystalline substance that occurs in nature as the mineral mascagnite. It is soluble in water and insoluble in alcohol or liquid ammonia. ..... Click the link for more information. . Ammonium salts of weak acids are readily decomposed into the acid and ammonia. Ammonium carbonate, (NH3)2CO3·H2O, is a colorless-to-white crystalline solid commonly known as smelling salts; in water solution it is sometimes called aromatic spirits of ammonia. Ammonia reacts with certain metal ions to form complex ions called ammines. Ammonia also reacts with Lewis acids (electron acceptors), e.g., sulfur dioxide or trioxide or boron trifluoride.

Another kind of reaction, commonly called ammonolysis, occurs when one or more of the hydrogen atoms in the ammonia molecule is replaced by some other atom or radical. Chlorine gas, Cl2, reacts directly with ammonia to form monochloramine, NH2Cl, and hydrogen chloride, HCl. Products of such ammonolyses include amides, amines, imides, imines, and nitrides. Ammonia also takes part in oxidation and reduction oxidation and reduction, complementary chemical reactions characterized by the loss or gain, respectively, of one or more electrons by an atom or molecule. Originally the term oxidation ..... Click the link for more information. reactions. It burns in oxygen to form nitrogen gas, N2, and water. In the presence of a catalyst (e.g., platinum) it is oxidized in air to form water and nitric oxide, NO. It reduces hot-metal oxides to the metal (e.g., cupric oxide to copper). Production Ammonia is prepared commercially in vast quantities. The major method of production is the Haber process Haber process , commercial process for the synthesis of ammonia, NH3.

Pure hydrogen and nitrogen gases are mixed in the appropriate proportion, heated to between 450&degC; and 600&degC;, compressed to about 1,000 atmospheres pressure, and passed over a catalyst. ..... Click the link for more information. , in which nitrogen is combined directly with hydrogen at high temperatures and pressures in the presence of a catalyst. It is obtained as a byproduct of the destructive distillation of coal. Ammonia is also prepared synthetically by the cyanamide process: nitrogen gas combines with calcium carbide, CaC2, at high temperatures to form calcium cyanamide, CaCN2, and carbon; the calcium cyanamide reacts with steam to form calcium carbonate, CaCO3, and ammonia. For use in the laboratory, ammonia is prepared by heating an ammonium salt with a strong base. It can also be prepared by reacting a metal nitride with water. Uses Ammonia solutions are used to clean, bleach, and deodorize; to etch aluminum; to saponify (hydolyze) oils and fats; and in chemical manufacture.

The ammonia sold for household use is a dilute water solution of ammonia in which ammonium hydroxide is the active cleansing agent. It should be used with caution since it can attack the skin and eyes. The vapors are especially irritating—prolonged exposure and inhalation cause serious injury and may be fatal. Water solutions of ammonia are also called ammonium hydrate, aqua ammonia, or ammonia water; the solution may contain up to 30% ammonium hydroxide by weight at room temperature and pressure. The major use of ammonia and its compounds is as fertilizers fertilizer, organic or inorganic material containing one or more of the nutrients—mainly nitrogen, phosphorus, and potassium, and other essential elements required for plant growth. ..... Click the link for more information. . Ammonia is also used in large amounts in the Ostwald process (see Ostwald, Wilhelm Ostwald, Wilhelm , 1853–1932, German physical chemist and natural philosopher, b. Riga, Latvia. He was professor of chemistry and director of the chemical laboratory (1886–1906) at the Univ. of Leipzig. ..... Click the link for more information.

) for the synthesis of nitric acid; in the Solvay process Solvay process [for Ernest Solvay], commercial process for the manufacture of sodium carbonate (washing soda). Ammonia and carbon dioxide are passed into a saturated sodium chloride solution to form soluble ammonium hydrogen carbonate, which reacts with the sodium chloride to ..... Click the link for more information. for the synthesis of sodium carbonate; in the synthesis of numerous organic compounds used as dyes, drugs, and in plastics; and in various metallurgical processes. Ammonia (NH3) the simplest chemical compound of nitrogen and hydrogen. Ammonia is one of the most important products of the chemical industry; the synthesis of ammonia from hydrogen and atmospheric nitrogen is the basic method for obtaining so-called fixed nitrogen. In nature ammonia is formed during the decay of nitrogen-containing organic compounds. The name “ammonia” is an abbreviation of the Greek hals ammoniakos or the Latin sal ammoniacus; this was the name given to ammonium chloride, which was produced at the oasis Ammonium (now Siwa) in the Libyan desert. Physical and chemical properties Ammonia is a colorless gas with a sharp, suffocating odor and a pungent taste.

The density of gaseous ammonia at 0°C and 101.3 kilonewtons (kN) per square meter (760 mm Hg) is 0.7714 kg/m3; it has a boiling point of -33.35°C, a melting point of -77.70°C, a critical temperature of 132.4°C, a critical pressure of 11.28 MN/m2 (115.0 kilograms-force [kgf] per square centimeter), a critical density of 235 kg/m3, and a heat of vaporization of 23.37 kilojoules per mole (5.581 kilocalories [kcal] per mole). A dry mixture of ammonia and air is capable of exploding. At room temperature the explosive limits lie between 15.5 percent and 28 percent ammonia. The range broadens with increased temperature. Ammonia is readily soluble in water (at 0°C one volume of water absorbs approximately 1,200 volumes of ammonia; at 20°C, about 700 volumes of ammonia).

At 20°C and 0.87 MN/m2 (8.9 kgf/cm2) ammonia is readily converted to a colorless liquid with a density of 681.4 kg/m3 and strong optical refractivity. Like water, liquid ammonia is strongly associated, mainly through the formation of hydrogen bonds. Liquid ammonia for all practical purposes does not conduct electricity. It is a good solvent of a large number of organic and inorganic compounds. Solid ammonia consists of colorless cubic crystals. The ammonia molecule has the form of a regular triangular pyramid with the nitrogen atom at the apex. The angles between the H—N—H bonds are 108°. Interatomic distance N—H is 1,015 Å, H—H is 1.64 Å. An interesting property of ammonia molecules is their ability to undergo structural inversion—that is, to “turn themselves inside out” by the passage of the nitrogen atom through the basal plane of the pyramid formed by the hydrogen atoms. Inversion is associated with emission of radiation of a very definite frequency. On the basis of this property an apparatus was constructed for determining time with very great precision (the molecular generator).

Such “molecular clocks” have made it possible to determine in particular that the duration of the terrestrial 24–hour day increases each year by 0.43 microseconds. The dipole moment of the ammonia molecule is 1.43 Debyes. Ammonia is diamagnetic because of the absence of unpaired electrons. Ammonia is an extremely reactive compound. Because of the presence of an unshared pair of electrons in the N molecule, addition reactions are especially marked and are easily realized by the ammonia molecule. Particularly important is the reaction in which a proton is added to the ammonia molecule, leading to the formation of the ammonium ion, NH4+, which in compounds with the anions of acids behaves like the ions of the alkali metals. When ammonia is dissolved in water, such reactions occur with the formation of the weak base ammonium hydroxide, NH4OH; they also occur when ammonia interacts directly with acids. A common addition reaction is the formation of ammoniates by the action of gaseous or liquid ammonia on salts. Substitution reactions are also characteristic for ammonia.

Depending on conditions, alkali and alkali earth metals react with liquid and gaseous ammonia, forming nitrides (Na3N) or amides (NaNH2). Ammonia also reacts with sulfur, halogens, carbon, C02, and other substances. Under ordinary conditions ammonia is quite resistant to oxidizing agents. However, when ignited, it burns in an oxygen atmosphere, forming water and free nitrogen. Catalytic oxidation of ammonia produces nitrogen oxides, which are then converted to nitric acid. Production and use Ammonia may be produced under laboratory conditions by displacing it from ammonium salts with strong alkalis according to the following equation: 2NH4C1 + Ca(OH)2 = 2NH3 + CaCl2 + 2H20. The oldest industrial method of producing ammonia is to separate it out from the gases emitted in the coking of coal. The principal modern method for industrial production of ammonia is its synthesis from the elements nitrogen and hydrogen, as proposed by the German chemist F. Haber in 1908. The most widespread and economical method for obtaining crude gas for the synthesis of ammonia is the conversion of hydrocarbon gases.

The initial raw material for this process may be natural gas, gaseous by-products of petroleum refining, or residual gases from the production of acetylene. The essence of the conversion method of obtaining a nitrogen-hydrogen mixture consists in the decomposition at high temperatures of methane and its homologues to hydrogen and carbon monoxide by the oxidizing agents water vapor and oxygen. Atmospheric air or air enriched with oxygen is added to the converted gas during this process. The synthesis of ammonia from its elements (N2 + 3H2 ⇌ 2NH3 + 92.1 kJ; 1 kJ=0.24 kcal) takes place with generation of heat and decrease in volume. From the point of view of equilibrium the most favorable conditions for the formation of ammonia are the lowest possible temperature and the highest possible pressure. Without catalysts the synthesis reaction of ammonia will not take place at all. In industry iron catalysts obtained from the reduction of molten oxides of iron, Fe304, with activators (A1203, K20, CaO, Si02, and sometimes MgO) are used exclusively.

An important step in the synthesis is the purification of the gaseous mixture from catalytic poisons, which include substances containing S, O2, Se, P, As, water vapor, and CO. Methods for the production of synthetic ammonia are designated according to the pressure applied: low-pressure (10–15 MN/m2), medium-pressure (25–30 MN/m2), and high-pressure (50–100 MN/m2) systems. Medium-pressure systems (30 MN/m2 and 500°C, 1 MN/m2 being approximately equal to 10 kgf/cm2) are the most widespread. Multiple circulation of the nitrogen-hydrogen mixture—the ammonia condensing cycle—is used to increase the utilization of gases in modern systems of ammonia synthesis (see Figure 1). Figure 1. Plant for ammonia synthesis (technological schema) Fresh gas (nitrogen-hydrogen mixture) and nonreacted, so-called circulating, gases first enter the filter (1), where they are cleansed of impurities, then go to the intertubular space of the condenser column (2), giving up their heat to the gas moving through the pipes of the column.

Farther on, the gases pass through the condenser (3), in which they are further cooled and in which ammonia carried by the circulating gases is condensed. From the condenser the cooled mixture of gases and condensed ammonia goes to the distributing section (separator) of the condensation column, where liquid ammonia is separated and carried along the pipe to the reservoir (9) as a finished product. Gaseous ammonia emerging from the evaporator is freed of drops of liquid ammonia going through the spray trap (4) and is directed to the reprocessing plant or to the refrigeration plant for condensation. Gases freed of ammonia go from the separator to the synthesizing column (5). Inside the synthesizing column is a catalyst compartment with tubular or shelved packing and a heat exchanger. Gases interact on passing through the synthesizing column; the gaseous mixture emerging from the column contains 15–20 percent ammonia. Farther along, the gases enter the condenser (6), in which the condensation of ammonia also occurs.

Liquid ammonia is separated out in the separator (7) and enters the reservoir, while the nonreacted gases are circulated by the pump (8) to the filter for mixing with a fresh nitrogen-hydrogen feed. Ammonia is used to produce nitric acid, nitrogen-containing salts, urea, hydrogen cyanide, and soda by the ammonia method. Because liquid ammonia has a high heat of evaporation, it serves as a working medium in refrigeration machines. Liquid ammonia and its aqueous solutions are used as liquid fertilizers. Large quantities of ammonia are used for the ammoniation of superphosphates and fertilizer mixtures. Ammonia is poisonous. It produces strong irritation of the mucous membranes. Acute ammonia poisoning affects the eyes and respiratory passages and causes dyspnea and lung inflammation. The highest permissible concentration of ammonia in the air of industrial installations is considered to be 0.02 g/m3. In the USSR ammonia is kept in steel cylinders painted yellow with the black inscription “ammonia.” REFERENCE Volatile alkali | Article about Volatile alkali by The Free Dictionary Volatile alkali | Article about Volatile alkali by The Free Dictionary Also found in: Dictionary , Thesaurus , Medical , Wikipedia .

ammonia, chemical compound, NH3, colorless gas that is about one half as dense as air at ordinary temperatures and pressures. It has a characteristic pungent, penetrating odor. Ammonia forms a minute proportion of the atmosphere; it is found in volcanic gases and as a product of decomposition of animal and vegetable matter. Because ammonia was formerly obtained by destructive distillation of horns and hooves of animals, its water solution was called spirits of hartshorn. Ammonia has also been called alkaline air and volatile alkali. Properties Anhydrous (water-free) ammonia gas is easily liquefied under pressure (at 20&degC; liquid ammonia has a vapor pressure of about 120 lb per sq in.) It is extremely soluble in water; one volume of water dissolves about 1,200 volumes of the gas at 0&degC; (90 grams of ammonia in 100 cc of water), but only about 700 volumes at room temperature and still less at higher temperatures. The solution is alkaline because much of the dissolved ammonia reacts with water, H2O, to form ammonium hydroxide, NH4OH, a weak base.

Liquid ammonia is used in the chemical laboratory as a solvent. It is a better solvent for ionic and polar compounds than ethanol, but not as good as water; it is a better solvent for nonpolar covalent compounds than water, but not as good as ethanol. It dissolves alkali metals and barium, calcium, and strontium by forming an unstable blue solution containing the metal ion and free electrons that slowly decomposes, releasing hydrogen and forming the metal amide. Compared to water, liquid ammonia is less likely to release protons (H+ ions), is more likely to take up protons (to form NH4+ ions), and is a stronger reducing agent. Because strong acids react with it, it does not allow strongly acidic solutions, but it dissolves many alkalies to form strongly basic solutions. Ammonia takes part in many chemical reactions. Ammonia reacts with strong acids to form stable ammonium salts: with hydrogen chloride it forms ammonium chloride ammonium chloride , chemical compound, NH4Cl, a white or colorless, odorless, water-soluble, cubic crystalline salt with a biting taste, commonly known as sal ammoniac. ..... Click the link for more information.

; with nitric acid, ammonium nitrate ammonium nitrate, chemical compound, NH4NO3, that exists as colorless, rhombohedral crystals at room temperature but changes to monoclinic crystals when heated above 32&degC;. It is extremely soluble in water and soluble in alcohol and liquid ammonia. ..... Click the link for more information. ; and with sulfuric acid, ammonium sulfate ammonium sulfate, chemical compound, (NH4)2SO4, a colorless-to-gray, rhombohedral crystalline substance that occurs in nature as the mineral mascagnite. It is soluble in water and insoluble in alcohol or liquid ammonia. ..... Click the link for more information. . Ammonium salts of weak acids are readily decomposed into the acid and ammonia. Ammonium carbonate, (NH3)2CO3·H2O, is a colorless-to-white crystalline solid commonly known as smelling salts; in water solution it is sometimes called aromatic spirits of ammonia. Ammonia reacts with certain metal ions to form complex ions called ammines. Ammonia also reacts with Lewis acids (electron acceptors), e.g., sulfur dioxide or trioxide or boron trifluoride.

Another kind of reaction, commonly called ammonolysis, occurs when one or more of the hydrogen atoms in the ammonia molecule is replaced by some other atom or radical. Chlorine gas, Cl2, reacts directly with ammonia to form monochloramine, NH2Cl, and hydrogen chloride, HCl. Products of such ammonolyses include amides, amines, imides, imines, and nitrides. Ammonia also takes part in oxidation and reduction oxidation and reduction, complementary chemical reactions characterized by the loss or gain, respectively, of one or more electrons by an atom or molecule. Originally the term oxidation ..... Click the link for more information. reactions. It burns in oxygen to form nitrogen gas, N2, and water. In the presence of a catalyst (e.g., platinum) it is oxidized in air to form water and nitric oxide, NO. It reduces hot-metal oxides to the metal (e.g., cupric oxide to copper). Production Ammonia is prepared commercially in vast quantities. The major method of production is the Haber process Haber process , commercial process for the synthesis of ammonia, NH3.

Pure hydrogen and nitrogen gases are mixed in the appropriate proportion, heated to between 450&degC; and 600&degC;, compressed to about 1,000 atmospheres pressure, and passed over a catalyst. ..... Click the link for more information. , in which nitrogen is combined directly with hydrogen at high temperatures and pressures in the presence of a catalyst. It is obtained as a byproduct of the destructive distillation of coal. Ammonia is also prepared synthetically by the cyanamide process: nitrogen gas combines with calcium carbide, CaC2, at high temperatures to form calcium cyanamide, CaCN2, and carbon; the calcium cyanamide reacts with steam to form calcium carbonate, CaCO3, and ammonia. For use in the laboratory, ammonia is prepared by heating an ammonium salt with a strong base. It can also be prepared by reacting a metal nitride with water. Uses Ammonia solutions are used to clean, bleach, and deodorize; to etch aluminum; to saponify (hydolyze) oils and fats; and in chemical manufacture.

The ammonia sold for household use is a dilute water solution of ammonia in which ammonium hydroxide is the active cleansing agent. It should be used with caution since it can attack the skin and eyes. The vapors are especially irritating—prolonged exposure and inhalation cause serious injury and may be fatal. Water solutions of ammonia are also called ammonium hydrate, aqua ammonia, or ammonia water; the solution may contain up to 30% ammonium hydroxide by weight at room temperature and pressure. The major use of ammonia and its compounds is as fertilizers fertilizer, organic or inorganic material containing one or more of the nutrients—mainly nitrogen, phosphorus, and potassium, and other essential elements required for plant growth. ..... Click the link for more information. . Ammonia is also used in large amounts in the Ostwald process (see Ostwald, Wilhelm Ostwald, Wilhelm , 1853–1932, German physical chemist and natural philosopher, b. Riga, Latvia. He was professor of chemistry and director of the chemical laboratory (1886–1906) at the Univ. of Leipzig. ..... Click the link for more information.

) for the synthesis of nitric acid; in the Solvay process Solvay process [for Ernest Solvay], commercial process for the manufacture of sodium carbonate (washing soda). Ammonia and carbon dioxide are passed into a saturated sodium chloride solution to form soluble ammonium hydrogen carbonate, which reacts with the sodium chloride to ..... Click the link for more information. for the synthesis of sodium carbonate; in the synthesis of numerous organic compounds used as dyes, drugs, and in plastics; and in various metallurgical processes. Ammonia (NH3) the simplest chemical compound of nitrogen and hydrogen. Ammonia is one of the most important products of the chemical industry; the synthesis of ammonia from hydrogen and atmospheric nitrogen is the basic method for obtaining so-called fixed nitrogen. In nature ammonia is formed during the decay of nitrogen-containing organic compounds. The name “ammonia” is an abbreviation of the Greek hals ammoniakos or the Latin sal ammoniacus; this was the name given to ammonium chloride, which was produced at the oasis Ammonium (now Siwa) in the Libyan desert. Physical and chemical properties Ammonia is a colorless gas with a sharp, suffocating odor and a pungent taste.

The density of gaseous ammonia at 0°C and 101.3 kilonewtons (kN) per square meter (760 mm Hg) is 0.7714 kg/m3; it has a boiling point of -33.35°C, a melting point of -77.70°C, a critical temperature of 132.4°C, a critical pressure of 11.28 MN/m2 (115.0 kilograms-force [kgf] per square centimeter), a critical density of 235 kg/m3, and a heat of vaporization of 23.37 kilojoules per mole (5.581 kilocalories [kcal] per mole). A dry mixture of ammonia and air is capable of exploding. At room temperature the explosive limits lie between 15.5 percent and 28 percent ammonia. The range broadens with increased temperature. Ammonia is readily soluble in water (at 0°C one volume of water absorbs approximately 1,200 volumes of ammonia; at 20°C, about 700 volumes of ammonia).

At 20°C and 0.87 MN/m2 (8.9 kgf/cm2) ammonia is readily converted to a colorless liquid with a density of 681.4 kg/m3 and strong optical refractivity. Like water, liquid ammonia is strongly associated, mainly through the formation of hydrogen bonds. Liquid ammonia for all practical purposes does not conduct electricity. It is a good solvent of a large number of organic and inorganic compounds. Solid ammonia consists of colorless cubic crystals. The ammonia molecule has the form of a regular triangular pyramid with the nitrogen atom at the apex. The angles between the H—N—H bonds are 108°. Interatomic distance N—H is 1,015 Å, H—H is 1.64 Å. An interesting property of ammonia molecules is their ability to undergo structural inversion—that is, to “turn themselves inside out” by the passage of the nitrogen atom through the basal plane of the pyramid formed by the hydrogen atoms. Inversion is associated with emission of radiation of a very definite frequency. On the basis of this property an apparatus was constructed for determining time with very great precision (the molecular generator).

Such “molecular clocks” have made it possible to determine in particular that the duration of the terrestrial 24–hour day increases each year by 0.43 microseconds. The dipole moment of the ammonia molecule is 1.43 Debyes. Ammonia is diamagnetic because of the absence of unpaired electrons. Ammonia is an extremely reactive compound. Because of the presence of an unshared pair of electrons in the N molecule, addition reactions are especially marked and are easily realized by the ammonia molecule. Particularly important is the reaction in which a proton is added to the ammonia molecule, leading to the formation of the ammonium ion, NH4+, which in compounds with the anions of acids behaves like the ions of the alkali metals. When ammonia is dissolved in water, such reactions occur with the formation of the weak base ammonium hydroxide, NH4OH; they also occur when ammonia interacts directly with acids. A common addition reaction is the formation of ammoniates by the action of gaseous or liquid ammonia on salts. Substitution reactions are also characteristic for ammonia.

Depending on conditions, alkali and alkali earth metals react with liquid and gaseous ammonia, forming nitrides (Na3N) or amides (NaNH2). Ammonia also reacts with sulfur, halogens, carbon, C02, and other substances. Under ordinary conditions ammonia is quite resistant to oxidizing agents. However, when ignited, it burns in an oxygen atmosphere, forming water and free nitrogen. Catalytic oxidation of ammonia produces nitrogen oxides, which are then converted to nitric acid. Production and use Ammonia may be produced under laboratory conditions by displacing it from ammonium salts with strong alkalis according to the following equation: 2NH4C1 + Ca(OH)2 = 2NH3 + CaCl2 + 2H20. The oldest industrial method of producing ammonia is to separate it out from the gases emitted in the coking of coal. The principal modern method for industrial production of ammonia is its synthesis from the elements nitrogen and hydrogen, as proposed by the German chemist F. Haber in 1908. The most widespread and economical method for obtaining crude gas for the synthesis of ammonia is the conversion of hydrocarbon gases.

The initial raw material for this process may be natural gas, gaseous by-products of petroleum refining, or residual gases from the production of acetylene. The essence of the conversion method of obtaining a nitrogen-hydrogen mixture consists in the decomposition at high temperatures of methane and its homologues to hydrogen and carbon monoxide by the oxidizing agents water vapor and oxygen. Atmospheric air or air enriched with oxygen is added to the converted gas during this process. The synthesis of ammonia from its elements (N2 + 3H2 ⇌ 2NH3 + 92.1 kJ; 1 kJ=0.24 kcal) takes place with generation of heat and decrease in volume. From the point of view of equilibrium the most favorable conditions for the formation of ammonia are the lowest possible temperature and the highest possible pressure. Without catalysts the synthesis reaction of ammonia will not take place at all. In industry iron catalysts obtained from the reduction of molten oxides of iron, Fe304, with activators (A1203, K20, CaO, Si02, and sometimes MgO) are used exclusively.

An important step in the synthesis is the purification of the gaseous mixture from catalytic poisons, which include substances containing S, O2, Se, P, As, water vapor, and CO. Methods for the production of synthetic ammonia are designated according to the pressure applied: low-pressure (10–15 MN/m2), medium-pressure (25–30 MN/m2), and high-pressure (50–100 MN/m2) systems. Medium-pressure systems (30 MN/m2 and 500°C, 1 MN/m2 being approximately equal to 10 kgf/cm2) are the most widespread. Multiple circulation of the nitrogen-hydrogen mixture—the ammonia condensing cycle—is used to increase the utilization of gases in modern systems of ammonia synthesis (see Figure 1). Figure 1. Plant for ammonia synthesis (technological schema) Fresh gas (nitrogen-hydrogen mixture) and nonreacted, so-called circulating, gases first enter the filter (1), where they are cleansed of impurities, then go to the intertubular space of the condenser column (2), giving up their heat to the gas moving through the pipes of the column.

Farther on, the gases pass through the condenser (3), in which they are further cooled and in which ammonia carried by the circulating gases is condensed. From the condenser the cooled mixture of gases and condensed ammonia goes to the distributing section (separator) of the condensation column, where liquid ammonia is separated and carried along the pipe to the reservoir (9) as a finished product. Gaseous ammonia emerging from the evaporator is freed of drops of liquid ammonia going through the spray trap (4) and is directed to the reprocessing plant or to the refrigeration plant for condensation. Gases freed of ammonia go from the separator to the synthesizing column (5). Inside the synthesizing column is a catalyst compartment with tubular or shelved packing and a heat exchanger. Gases interact on passing through the synthesizing column; the gaseous mixture emerging from the column contains 15–20 percent ammonia. Farther along, the gases enter the condenser (6), in which the condensation of ammonia also occurs.

Liquid ammonia is separated out in the separator (7) and enters the reservoir, while the nonreacted gases are circulated by the pump (8) to the filter for mixing with a fresh nitrogen-hydrogen feed. Ammonia is used to produce nitric acid, nitrogen-containing salts, urea, hydrogen cyanide, and soda by the ammonia method. Because liquid ammonia has a high heat of evaporation, it serves as a working medium in refrigeration machines. Liquid ammonia and its aqueous solutions are used as liquid fertilizers. Large quantities of ammonia are used for the ammoniation of superphosphates and fertilizer mixtures. Ammonia is poisonous. It produces strong irritation of the mucous membranes. Acute ammonia poisoning affects the eyes and respiratory passages and causes dyspnea and lung inflammation. The highest permissible concentration of ammonia in the air of industrial installations is considered to be 0.02 g/m3.

In the USSR ammonia is kept in steel cylinders painted yellow with the black inscription “ammonia.” REFERENCE Ammonia-solution | Define Ammonia-solution at Dictionary.com C18: from New Latin, from Latin (sal) ammōniacus (sal) ammoniac1 Collins English Dictionary - Complete & Unabridged 2012 Digital Edition © William Collins Sons & Co. Ltd. 1979, 1986 © HarperCollins Publishers 1998, 2000, 2003, 2005, 2006, 2007, 2009, 2012 Word Origin and History for ammonia-solution Expand ammonia n.

1799, Modern Latin, coined 1782 by Swedish chemist Torbern Bergman (1735-1784) for gas obtained from sal ammoniac, salt deposits containing ammonium chloride found near temple of Jupiter Ammon (from Egyptian God Amun) in Libya, from Greek ammoniakos "belonging to Ammon." The shrine was ancient already in Augustus' day, and the salts were prepared "from the sands where the camels waited while their masters prayed for good omens" [Shipley]. There also was a gum form of sal ammoniac, from a wild plant that grew near the shrine, and across North Africa and Asia. A less likely theory traces the name to Greek Armeniakon "Armenian," because the substance also was found in Armenia. Also known as spirit of hartshorn and volatile or animal alkali. Online Etymology Dictionary, © 2010 Douglas Harper Glossary Glossary saccharum saturni: sugar of lead ; see also Saturn sal ... ... aeratus (or saleratus, literally aerated salt): potassium hydrogen carbonate, KHCO3. ... albus: borax ...

ammoniac: ammonium chloride, NH4Cl [ Black , Fahrenheit , Scheele , Wurtz , et al.]; also sal armoniack [ Helmont ] ... commune: common salt, i.e., sodium chloride, NaCl [ Scheele ]; also ; also sal fossile, sal marinum ... de duobus: potassium sulfate, K2SO4 ( vitriolate of tartar ) ... enixum: potassium hydrogen sulfate (KHSO4) ... nitrum or ... nitri: nitre . [ Mayow ] ... sapientiae: mercury(II) ammonium chloride, HgNH2Cl; literally, "salt of the wise". (white precipitate) ... volatile: ammonium carbonate, (NH4)2CO3 -peter or -petre: potassium nitrate, KNO3 ( nitre ). [ Bacon , Helmont , T. Thomson ] ... of tin: tin(II) chloride, SnCl2 urinous ...: (sel urineux) an ammonium salt. Occasionally any alkaline salt. ...

of wormwood: potassium carbonate, K2CO3 Saturn: In astrological and alchemical thought, the seven heavenly bodies known to the ancients were associated with seven metals also known in antiquity. Saturn was associated with lead (plumbum) Scheele's green: an acidic copper(II) arsenite, CuHAsO3, named for Carl Wilhelm Scheele . Schlippe's salt: sodium sulfantimonate, Na3SbS4.9H2O, named for Carl Friedrich von Schlippe. Sch�llkopf's acid: apparently, Sch�llkopf had three. 1-naphthol-4,8-disulfonic acid, 1-naphthylamine-4,8-disulfonic acid, and 1-naphthylamine-8-sulfonic acid. (Click here for structures.) scruple: See apothecary measures . Seignette's salt: see rochelle salt . Peter Seignette was an apothecary at Rochelle. Seven planets, seven metals: In astrological and alchemical thought, the seven heavenly bodies known to the ancients were associated with seven metals also known in antiquity.

The associations were: Sun (Sol) siliceous earth: silicon dioxide, SiO2. [ Lavoisier , Scheele ] silver ... black ...: stephanite, a native silver antimony sulfide, 5Ag2S.Sb2S fulminating ...: silver nitride, Ag3N, an explosive solid; distinct from silver fulminate, Ag2C2N2O2, which is also explosive ... glance: argentite, silver sulfide, Ag2S. (See glance .) horn ...: a native silver chloride, AgCl (argentum cornu) ruby ...: proustite, Ag3AsS3 soda: sodium carbonate, Na2CO3 (washing soda), or sodium hydrogen carbonate, NaHCO3 (baking soda) [ Dalton , Lavoisier , Prout , Rayleigh ]. Caustic soda was sodium hydroxide, NaOH. [ Mendeleev ]. See also fossil alkali , marine alkali , common mineral alkali .

sorrel salt: potassium hydrogen oxalate, KHC2O4 (sal acetosella, salt of lemon) Spanish white: bismuth oxychloride, BiOCl, or oxynitrate, BiONO3 spirit (spiritus): an essence or extract that can be prepared from another substance as by distillation. If not specified, spirits refer to alcohol (ethanol). ... of alum: sulfuric acid, H2SO4 colonial or Columbian ...: methanol, CH3OH ... of hartshorn: ammonia, NH3, or its aqueous solution (formerly prepared from animal horns or hooves); see also salt of hartshorn . See alkaline air , volatile alkali . [ Black ] ... of nitre: nitric acid, HNO3 ( aqua fortis , nitrous acid , acid spirit of nitre) [ Cavendish , Fahrenheit , Mayow , Priestley ] or ethyl nitrite, C2H5NO2, also known as the sweet spirit of nitre or nitrous ether . See nitre . pyroacetic ...: acetone, (CH3)2CO sulphurous acid or sulphurous gas: formerly meant sulfur dioxide, SO2.

[ Avogadro , Gay-Lussac , Lavoisier , Prout , T. Thomson , et al.] Sun (Sol): In astrological and alchemical thought, the seven heavenly bodies known to the ancients were associated with seven metals also known in antiquity. The sun was associated with gold (aurum). sweet salt: sodium chlorite, NaClO2. Sylvius's febrifuge salt: potassium chloride, KCl; named for the iatrochemist Franciscus Sylvius tartar: (tartar of wine) potassium hydrogen tartrate, KHC4H4O6 [ Stahl ] cream of ... (cremor tartari): tartar purified into small white crystals. ... emetic: potassium antimonyl tartrate, KSbOC4H4O6.1/2H2O oil of ...: a saturated solution of potassium carbonate, K2CO3 [ Lavoisier ] salt of ...: solid potassium carbonate [ Black , Cavendish , Rey , Stahl ] vitriolate of ...

(or vitriolated): potassium sulfate, K2SO4 [ Priestley , Scheele ] (sal de duobus) tectum argenti: bismuth (construed as silver not completely formed in the earth) terra ...: earth ... ponderosa ("heavy earth"), barium oxide, BaO ... ponderosa aerata ("aerated heavy earth"), barium carbonate, BaCO3 Thénard's blue: blue cobalt aluminate, Co(AlO2)2, named for Louis-Jacques Thénard . thorium ... See table . ... A: an isotope of polonium produced in thorium decay, namely 216Po (half-life = 0.15 s).[ Soddy ] ... C: The names of two radioisotopes, both produced in thorium decay, included thorium C. Simple thorium C was an isotope of bismuth, namely 212Bi (half-life = 61 min); thorium C' was an isotope of polonium, namely 212Po (half-life = 0.3 µs) [ Rutherford , Soddy ] ...

D: an isotope of thallium produced in thorium decay, namely 208Tl (half-life = 3 min). [Soddy 1 & 2 ] ... X: an isotope of radium produced in thorium decay, namely 224Ra (half-life = 3.6 d). [ Rutherford, Soddy ] thymol blue: thymolsulphonphthalein, C27H30O5S, an acid-base indicator that changes from pink to yellow as the pH is raised through 2.2 and then to blue as the pH is raised through 8.8 trona: natural sodium carbonate/bicarbonate, Na2CO3.NaHCO3.2H2O Turnbull's blue: ferroferricyanide, Fe3[Fe(CN)6]2, also known as insoluble Prussian blue turbith mineral (or turpeth): basic sulfate of mercury, HgSO4.2HgO.

[ Cavendish , Lavoisier , Priestley ] tyrian purple: 6,6'-dibromoindigotin , C16H8N2O2Br2, an important dye of the ancient Mediterranean. uranium ... See table . ... I: is simply the most abundant isotope of uranium, 238U. ... II: an isotope of uranium produced in uranium decay, namely 234U (half-life = 2.5x105 y). [Soddy 1 , 2 , & 3 ] ... X: There were two uranium X produced in uranium decay. Uranium X1 (simply uranium X before the discovery of uranium X2) was an isotope of thorium, namely 234Th (half-life = 24 d); uranium X2 was an isotope of protactinium 234Pa. [Crookes; Rutherford ; Soddy 1 , 2 , & 3 ] ... yellow: sodium uranate, Na2UO4, a pigment used in glass and ceramics urinous ... ... air: (aer urinosa) ammonia. See alkaline air ...

salt: (sel urineux) an ammonium salt, or occasionally, any alkaline salt vegetable alkali: usually crude or purified potassium carbonate, K2CO3 ( pearl ash ), sometimes specified as mild vegetable alkali or fixed vegetable alkali. Caustic vegetable alkali is potassium hydroxide. [ Davy ] Venus: In astrological and alchemical thought, the seven heavenly bodies known to the ancients were associated with seven metals also known in antiquity. Venus was associated with copper (cuprum). virginium (Vi or Vm): a name proposed for element 87 (francium) in a report of detection of the element whose validity was ultimately not recognized. verdigris: basic copper acetate, used as a pigment from green to blue. Literally "green of Greece" in French; however, it was also called Spanish green . blue verdigris is copper(II) acetate, Cu(C2H3O2)2.H2O. vermilion: mercury(II) sulfide, HgS, a red pigment; also known as cinnabar. (See minium .) vis viva: energy.

The law of conservation of energy was originally phrased in terms of vis viva [ Clausius , Joule , Kelvin , Mayer ] vitamin (or sometimes vitamine, from "vital amine" [Funk]): an organic substance essential in small quantities to the normal health of an animal. Vitamins must typically be supplied to the animal through diet. The chemical names for some vitamins follow. For structures, see "Molecule of the Month" at Oxford University . ... A: retinol, C20H30O, a fat-soluble vitamin derived from carotenes ... B: a group of water-soluble, heat labile compounds that typically serve as co-enzymes. They include many examples that contain amine groups (as in "vital amine"). ... B1: thiamin (or thiamine), C12H17N4OSCl ... B2: riboflavin (or riboflavine), C17H20N4O6 ... B3: niacin (or nicotinic acid), C6H5NO2 ... B6: pyridoxin (or pyridoxine), C8H11NO3 ...

B12: cyanocobalamin (or cyanocobalamine), C63H90CoN14O14P ... Bc: folic acid, C19H19N7O6 ... C: ascorbic acid, C6H8O6, a water-soluble vitamin found in many fruits and green vegetables ... D: This fat-soluble vitamin consists of steroid derivatives including ergocalciferol, C28H44O, and cholecalciferol, C27H44O. ... E: This vitamin occurs in four naturally occuring forms, called α-, β-, γ-, and δ-tocopherol. The α form, C29H50O2, has the greatest activity; the β- and γ- forms have one fewer methyl group, and the δ- form two fewer. vitriol: a sulfate, especially iron sulfate; see copperas .

vitriolic acid: sulfuric acid, H2SO4 [ Black , Cavendish , Lavoisier , Priestley ], also known as oil of sulfur per campanum, oil of vitriol [ Black , Lavoisier , Scheele , Stahl ], and spirit of vitriol (spiritus vitrioli) [ Black , Scheele ]. vitriolic acid air (and sometimes vitriolic acid): sulfur dioxide, SO2, also known as sulphurous acid or sulphurous gas. blue vitriol: copper sulfate, CuSO4.5H2O, also roman vitriol green vitriol: iron(II) sulfate, FeSO4.7H2O red or rose vitriol: cobalt(II) sulfate, CoSO4.7H2O uranvitriol: a uranium sulfate white vitriol or salt of vitriol: zinc sulfate, ZnSO4.7H2O [ Scheele ]; also salt of vitriol volatile alkali: aqueous ammonia, NH3; see alkaline air , spirit of hartshorn . Concrete volatile alkali refers to ammonium carbonate, (NH4)2CO3.

[ Black , Cavendish , Lavoisier , Scheele , et al.] water glass (also soluble glass): a hydrated sodium silicate, Na2Si4O9.xH2O, either an amorphous solid or in thick aqueous solution, used as a binder or adhesive. wolfram: a name of Germanic origin originally applied to a native iron manganese tungstate and later to the element tungsten, hence the symbol W. xylenol blue: 1,4-dimethyl-5-hydroxybenzenesulfonphthalein, an acid-base indicator that changes from red to yellow as the pH is raised through 2 and then to blue as the pH is raised through 8.8. Go back to the previous part (M-R) of the Glossary. Back to the top of the Classic Chemistry site Carbonate Carbonate - Sodium Carbonate Ammonium Carbonate Ammonium carbonate is the commercial salt, formerly known as sal volatile or salt of hartshorn. Ammonium carbonate is used when crushed as a smelling salt. It can be crushed when needed in order to revive someone who has fainted.

» request a quote Copper Carbonate Copper(II) carbonate (often called copper carbonate or cupric carbonate) is a blue-green compound (chemical formula CuCO3) forming part of the verdigris patina one sees on weathered brass, bronze, and copper. » request a quote Lithium Carbonate Lithium carbonate is a chemical compound with the formula Li2CO3. This colorless salt is widely used in the processing of metal oxide and has received attention for its use in psychiatry. » request a quote Magnesium Carbonate Magnesium carbonate, MgCO3, is a white solid that occurs in nature as a mineral. Several hydrated and basic forms of magnesium carbonate also exist as minerals. In addition, MgCO3 has a variety of uses. » request a quote Potassium Carbonate Potassium carbonate is a white salt, soluble in water (insoluble in alcohol), which forms a strongly alkaline solution. It can be made as the product of potassium hydroxide's absorbent reaction with carbon dioxide. » request a quote Sodium Carbonate Sodium carbonate (also known as washing soda, soda crystals or soda ash), Na2CO3, is a sodium salt of carbonic acid.

It most commonly occurs as a crystalline heptahydrate, which readily effloresces to form a white powder, the monohydrate; and is domestically well known for its everyday use as a water softener. Smelling Salts (3.5e Equipment) - D&D Wiki Smelling Salts (3.5e Equipment) Smelling Salts[ edit ] Smelling salts are chemical compounds used to arouse an unconscious person. Common alchemical items used as smelling salts included Sal Volatile (ammonium carbonate), Caustic Volatile Alkali (ammonium hydroxide), or a Spirit of Hartshorn (ammonia) dissolved in an alcohol solution. They are generally cheap and simple to produce for even amateur alchemists. Smelling salts give a +1 alchemical bonus to Heal checks performed on headaches, or on attempts to revive or wake an unconscious person. One vial costs 10 gp and weighs 1 lb.

Question: Sal volatile (spirit of hartshorn) is a solution commonly known as what?
Answer: Smelling salts